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adell [148]
3 years ago
8

If .00327 g of a gas dissolves in 0.376 L of water at 867 torr, what quantity of this gas (in grams) will dissolve at 759 torr?

Chemistry
1 answer:
Vinil7 [7]3 years ago
8 0

At 759 torr, 0.002 86 g of the gas will dissolve.

Henry’s law states:

c = k_{H}p, where

where K_{H} is a proportionality constant called the Henry's Law constant.

If we have the same solute in the same solvent at two different pressures  p_{1} and p_{2},  

c_{1} = k_{H}p_{1} and c_{2} = k_{H}p_{2}

Dividing the two equations, k_H cancels and we get

c_1/c_2 = p_1/p_2

<em>c</em>_2 = <em>c</em>_1 × <em>p</em>_2/<em>p</em>_1

The volumes of solvent are the same, so we can use the masses of the solute instead of concentrations.

∴ <em>c</em>_2 = 0.003 27 g × (759 torr/867 torr) = 0.002 86 g

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Copper is commonly mined as an ore with a variable percent composition of copper (II) sulfide. This ore is also sometimes referr
pantera1 [17]

Answer:

m_{CuO}=93.6gCuO

Explanation:

Hello,

In this case, the undergoing chemical reaction is:

CuS+\frac{3}{2} O_2\rightarrow CuO+SO_2

Thus, given the 1.00-kg of 12.5% ore, we can compute the theoretical yield of copper (II) oxide via stoichiometry:

m_{CuO}^{theoretical}=1.00kgCuS*\frac{1000gCuS}{1kgCuS} *\frac{12.5gCuS}{100gCuS} *\frac{1molCuS}{95.6gCuS} *\frac{1molCuO}{1molCuS} *\frac{79.5gCuO}{1molCuO} \\\\m_{CuO}^{theoretical}=103.95gCuO

Whereas the third factor accounts for the percent purity of the covellite. Then, given the percent yield, we can compute the actual yield by:

m_{CuO}=103.95gCuO*0.9\\\\m_{CuO}=93.6gCuO

Regards.

6 0
3 years ago
PLEASE HELP ME SOLVE THIS.Thank you so much!
Tju [1.3M]

Answer: The coefficients for the given reaction species are 1, 6, 2, 3.

Explanation:

The given reaction equation is as follows.

Cr_{2}O^{2-}_{7} + Cl^{-} \rightarrow Cr^{3+} + Cl_{2}

Now, the two half-reactions can be written as follows.

Reduction half-reaction: Cr_{2}O^{2-}_{7} + 3e^{-} \rightarrow Cr^{3+}

This will be balanced as follows.

Cr_{2}O^{2-}_{7} + 14H^{+} + 6e^{-} \rightarrow 2Cr^{3+} + 7H_{2}O ... (1)

Oxidation half-reaction: Cl^{-} \rightarrow Cl_{2} + 1e^{-}

This will be balanced as follows.

6Cl^{-} \rightarrow 3Cl_{2} + 6e^{-} ... (2)

Adding both equation (1) and (2) we will get the resulting equation as follows.

Cr_{2}O^{2-}_{7} + 14H^{+} + 6Cl^{-} \rightarrow 2Cr^{3+} + 3Cl_{2} + 7H_{2}O

Thus, we can conclude that coefficients for the given reaction species are 1, 6, 2, 3.

6 0
2 years ago
2) Calculate the mass(g) of the following substances:<br> b) 0.119 mole MgCl2
VARVARA [1.3K]

Answer:

MgCl2 = 24 + 2(35.5)

= 95

mass of substance = mol × molar mass

= 0.119 × 95

= 11.305 g

4 0
3 years ago
A manganese electrode was oxidized electrically. If the mass of the electrode decreased by 225 mg during the passage of 1580 cou
qwelly [4]

Answer:

<u>Oxidation state of Mn = +4</u>

Explanation:

Atomic mass of Mn = 55g/mol

From Faraday's law of electrolysis,

Electrochemical equivalent = \frac{mass}{charge}

i.e Z = \frac{m}{Q} = \frac{0.225g}{1580C} = 0.0001424 g/C

But Equivalent weight, E = atomic mass ÷ valency  = Z × 96,485

⇒ \frac{55}{valency} = 0.0001424 × 96,485

<u>∴ Valency of Mn = +4</u>

8 0
3 years ago
How many grams of water do you need to weigh if a reaction requires 5 moles of h2o
rewona [7]

One mole of water weighs 18 grams. H₂O is composed of 2H= 2 and 1 0=16 adding gives you 18. number of moles= mass/ Relative Molecular Mass

Therefore, mass= Relative Molecular Mass×number of moles

                           = 18×5 moles

                           = 90 grams

5 0
3 years ago
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